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Bezzdna [24]
3 years ago
7

Convert the average temperatures for each collected data point given below from °C to K. Plot the average cell potentials E (y-a

xis) vs T (x-axis). The plot should be approximately linear. Add a trendline to find the best linear fit and write down the y-intercept and slope (b and m from the linear equation) for the trendline below.
Average Temperature in °C - Average Cell Potential (V)

15 - 0.465
18 - 0.467
21 - 0.468
24 - 4.69
27 - 0.471
30 - 0.472
33 - 0.474

Chemistry
1 answer:
koban [17]3 years ago
7 0

Answer:

Explanation:

The equation of above line , y = 0.0005x+ 0.458

This can be compared with y = mx+c

Hence slope, m = 0.0005 and Y-intercept, c = 0.458

Or it can be plotted manually where straight line has to be drawn touching maximum number of data points. After drawing a straight linear line, we need to take any two points from the straight line and slope is calculated

Slope,

m = \frac{y_2-y_1}{x_2-x_1}

and y -intercept is calculated using extraplotting backwards such that it touches the Y-axis. the point where straight line touches Y-axis is Y-intercept (c).

Plot the average cell potentials E (y-axis) vs T (x-axis). image attached

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The following questions pertain to a system contains 122 g CO(g) in a 0.400 L container at -71.2 degrees C.
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a. P = 182 atm

Explanation:

Data Given:

amount of CO = 122g

Volume of CO = .400 L

Temperature of CO =  -71.2°C

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T =  -71.2 + 273

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To calculate Pressure by using ideal gas formula

                  PV = nRT

Rearrange the equation for Pressure

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where

P = pressure

V = Volume

T= Temperature

n = Number of moles

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For this we have to know the mole of the gas and the following formula will be used

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Molar mass of CO = 12 + 16 = 28 g/mol

Put values in equation 2

                no. of moles = 122 g / 28 g/mol

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Now put the value in formula (1) to calculate Pressure for CO

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So the pressure will be 182 atm

__________

b. Data Given:

Actual pressure exerted by CO = 145 atm

expected pressure exerted by CO = 182 atm

why the actual pressure is less than what would be expected = ?

Explanation:

This is because of the deviation from ideal behavior of real gases.

The real gases approach to ideal behavior under very high temperature and very low pressure.

But CO deviate from ideal behavior to give expected value for pressure, because it behave at high pressure and low temperature.

This non-ideal behavior is due to two postulate of ideal behavior

  • gas molecules have negligible volume
  • Gas molecules have negligible inter-molecular interaction

but these postulates not obeyed under real condition. so we calculated the pressure using ideal condition values for gas and obtained the expected value for pressure but the actual pressure value was detected under normal condition.

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